Diborano: diferenças entre revisões
Conteúdo apagado Conteúdo adicionado
m |
m +tag/corr (-dead refs, +cats) |
||
Linha 1:
{{em tradução|data=outubro de 2011}}
{{Info/Química
| verifiedrevid = 443635822
Linha 58 ⟶ 59:
==Estrutura e ligação==
[[Ficheiro:Diborane b2h6 bonding diagram.png|150px|left]]
A [[
<!--
Diborane adopts a D<sub>2h</sub> structure containing four terminal and two bridging hydrogen atoms. The model determined by [[molecular orbital theory]] indicates that the bonds between boron and the terminal hydrogen atoms are conventional 2-center, 2-electron [[covalent bond]]s. The bonding between the boron atoms and the bridging hydrogen atoms is, however, different from that in molecules such as hydrocarbons. Having used two electrons in bonding to the terminal hydrogen atoms, each boron has one [[valence electron]] remaining for additional bonding. The bridging hydrogen atoms provide one electron each. Thus the B<sub>2</sub>H<sub>2</sub> ring is held together with four electrons, an example of [[3-center-2-electron bond]]ing. This type of bond is sometimes called a 'banana bond'. The lengths of the B-H<sub>bridge</sub> bonds and the B-H<sub>terminal</sub> bonds are 1.33 and 1.19 Å respectively, and this difference in the lengths of these bonds reflects the difference in their strengths, the B-H<sub>bridge</sub> bonds being relatively weaker. The structure is [[isoelectronic]] with C<sub>2</sub>H<sub>6</sub><sup>2+</sup>, which would arise from the diprotonation of the planar molecule [[ethene]].<ref>{{ cite journal | journal = [[Journal of Physical Chemistry A|J. Phys. Chem. A]] | year = 2005 | volume = 109 | issue = 5 | pages = 798–801 | author = G. Rasul, G. K. S. Prakash, [[George Andrew Olah|G. A. Olah]] | doi = 10.1021/jp0404652 | title = Comparative ab Initio Study of the Structures and Stabilities of the Ethane Dication C<sub>2</sub>H<sub>6</sub><sup>2+</sup> and Its Silicon Analogues Si<sub>2</sub>H<sub>6</sub><sup>2+</sup> and CSiH<sub>6</sub><sup>2+</sup> | pmid = 16838949 }}</ref> Diborane is one of many compounds with such unusual bonding.<ref>{{cite journal | author= Laslo P | title= A Diborane Story | journal= Angewandte Chemie International Edition | year= 2000 | volume= 39 | pages= 2071–2072| doi= 10.1002/1521-3773(20000616)39:12<2071::AID-ANIE2071>3.0.CO;2-C | pmid=10941018 | issue= 12}} [http://www3.interscience.wiley.com/cgi-bin/abstract/72507084/ABSTRACT abstract]</ref>
Linha 122 ⟶ 125:
The toxic effects of diborane are primarily due to its irritant properties. Short-term exposure to diborane can cause a sensation of tightness of the chest, shortness of breath, cough, and wheezing. These signs and symptoms can occur immediately or be delayed for up to 24 hours. Skin and eye irritation can also occur. Studies in animals have shown that diborane causes the same type of effects observed in humans. {{Citation needed|date=September 2009}}
People exposed for a long time to low amounts of diborane have experienced respiratory irritation, [[seizures]], fatigue, [[drowsiness]], confusion, and occasional transient tremors.-->
{{Referências}}
==
* [http://www.inchem.org/documents/icsc/icsc/eics0432.htm International Chemical Safety Card 0432]
* [http://box27.bluehost.com/~edsanvil/wiki/index.php?title=Diborane Computational Chemistry Wiki]
Linha 140 ⟶ 136:
* [http://www.epa.gov/oppt/aegl/results65.htm U.S. EPA Acute Exposure Guideline Levels]
[[Categoria:Compostos de hidrogénio]]
▲-->[[Categoria:agentes redutores]]
[[ca:Diborà]]
|